Covers atomic energy levels, including ground and excited states, energy diagrams and the four quantum numbers, followed by the Pauli exclusion principle and its consequences for electron arrangement. Explains optical transitions by photon absorption and emission, with a formula, then compares emission, absorption and fluorescence spectroscopy for elemental analysis. Closes with molecular energy levels and the instruments used for atomic emission, absorption and fluorescence analysis and their main components.
Topic 31 of 42 in the MU Sofia syllabus for Physics (Medicine, Year 1). The free AceMed note covers it in 5 sections, about 308 words (2 min of reading), with 8 flashcards.
In this note
Atomic Spectra – Structure of Atoms
Atomic Energy Levels
Pauli Exclusion Principle
Optical Transitions Between Energy Levels
Atomic Spectral Analysis
Atomic Energy Levels
Ground State:
The lowest, most stable energy state of an atom.
Electrons here have minimum possible energy.
Excited State:
Achieved when an electron absorbs energy and moves to a higher orbital.
Less stable than the ground state.
Energy Diagrams:
Represent electronic energy levels visually.
Each line corresponds to a possible state of an electron in the atom.
Quantum Numbers:
Define electron position and properties:
nnn: Principal quantum number (energy level, size).
lll: Azimuthal/Angular momentum number (shape of orbital).
mmm: Magnetic quantum number (orientation).
sss: Spin quantum number (±½).
Pauli Exclusion Principle
Statement: No two identical fermions (electrons) can occupy the same quantum state simultaneously in an atom.
Implications:
Determines the electronic configuration of atoms.
Explains periodicity in chemical properties.
Governs the arrangement of electrons in orbitals.
Optical Transitions Between Energy Levels
Mechanism: Electrons move between energy levels by absorbing or emitting photons.
Absorption:
Electron absorbs a photon → jumps to a higher energy level.
Emission:
Electron returns to lower energy level → emits a photon.
Formula:
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